Free Chemical Bonding MCQs with Answers

• A. N
• B. CI
• C. O
• D. He

Explanation: He belongs to group 8A and has a stable electronic configuration.Electron affinity is inversely proportional to the stability of…

• A. Ionization energy of A is high and electron affinity of B is low
• B. Ionization energy of A is low and electron affinity of B is high
• C. Both the ionization energy and the electron affinity of A and B are high
• D. Both the ionization energy and the electron affinity of A and B are low

Explanation: Ionic compound is formed between the two atoms when one of them has low ionization energy so it can easily give away electrons and other…

• A. NaCI
• B. CsF
• C. KCI
• D. HF

Explanation: Strength of ionic character depends upon electronegativity difference. CsF has greatest electronegativity difference of 3.19 and maximum…

• A. OH-
• B. BF-4
• C. NH+4
• D. H3O+

Explanation: OH-(hydroxide ion) does not have a dative bond. It is an example of a negatively charged ion formed through ionic bonding.

• A. Nitride ion
• B. Chloronium ion
• C. Hydronium ion
• D. All of these

Explanation: Yes, the hydronium ion (H3O+) contains a dative bond. The hydronium ion is formed when a water molecule (H2O) donates a lone pair of…

• A. Ionic
• B. Polar covalent
• C. Non-polar covalent
• D. Metallic

Explanation: The bond between two atoms is non-polar covalent if electronegativity difference between them is zero or less than 0.5.The bond between…

• A. CS2
• B. CO2
• C. SO2
• D. BeCl2

Explanation: SO2 is a bent or V-shaped molecule. It has a bond angle of approximately 120 degrees between the sulfur atom (S) and the two oxygen atoms…

• A. CH4
• B. PCI5
• C. NH+4
• D. PCI3

Explanation: PCl3 has 3 single bonds with Cl and one lone pair.

• A. NH3, PH3
• B. BF3, AIH3
• C. H2O, C2H2
• D. CO2, SO2

Explanation: BF3 and AIH3 are trigonal planar because each has three bond pairs only (AB3 type).

• A. Linear
• B. Angular
• C. Pyramidal
• D. Tetrahedral

Explanation: NH2- ion has a total of 8 valence electrons. 2 pairs are bonding and 2 are non-bonding and stay confined to the Nitrogen atom.

• A. Trigonal planar
• B. Tetrahedral
• C. Trigonal pyramidal
• D. Angular

Explanation: Trigonal planar shape is only possible for AB3 type molecules.

• A. CH4 >H2O> NF3 > H2S
• B. H2S>H2O> CH4 > NF3
• C. CH4 > NF3>H2O>H2S
• D. CH4 >H2S> H2O > NF3

Explanation: CH4 (109.5°) > H2O (104.5°)> NF3 (102°) > H2S (92°)

• A. CO2
• B. PH3
• C. NO
• D. SO3

Explanation: SO3 is AB3 type with three bond pairs and no lone pair so it has perfect triangular structure.

• A. It doesn't address the shapes of the molecules
• B. It doesn't involve the criteria of bond formation
• C. It doesn't explain paramagnetic behavior of O2
• D. None of the above

Explanation: Paramagnetic behaviour of oxygen is explained by MOT not VBT.

• A. Sigma bond
• B. Pi bond
• C. Metallic bond
• D. Co-ordinate covalent bond

Explanation: End to end overlapping of orbitals is axial overlapping and is linear which results in sigma bond.

• A. Non-hybrid orbitals
• B. Hybrid orbitals
• C. Hybrid and non-hybrid orbitals
• D. Atomic orbital and hybrid orbital

Explanation: π-bonds are formed by parallel overlapping of un-hybrid orbitals.

• A. It does not explain paramagnetism of O2
• B. It does not explain odd electron system
• C. It could not explain tetravalency of carbon
• D. All of above

Explanation: VBT does not explain tetravalency of carbon atom but concept of hybridization does.

• A. s-s orbital
• B. p-p head on overlapping of orbitals
• C. s-p orbital
• D. p-p parallel overlapping of orbitals

Explanation: The Cl2 molecule is formed by the overlap of two chlorine atoms' atomic orbitals.

• A. Dissolution
• B. Resonance
• C. Hybridization
• D. Ionization

Explanation: The process in which the orbitals of different energies and shape mix with each other to give equivalent hybrid orbitals is called…

• A. NH+4
• B. NH2-
• C. NH3
• D. NO3-

Explanation: In NO3- (Nitrate ion), the central nitrogen atom is in a hybridization state of sp2.